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In a conductometric titration, small volume of titrant of higher concentration is added stepwise to a larger volume of titrate of much lower concentration, and the conductance is measured after each addition. The limiting ionic conductivity ( ₀ ) values (in mS m ^2 ~mol ⁻¹ ) for different ions in aqueous solutions are given below: For different combinations of titrates and titrants given in List-I, the graphs of 'con

Options

  1. AP -4, Q -3, R -2, ~S -5
  2. BP -2, Q -4, R -3, ~S -1
  3. CP -3, Q -4, R -2, ~S -5
  4. DP -4, Q -3, R -2, ~S -1

Correct answer

C. P -3, Q -4, R -2, ~S -5

Step-by-step solution

Option (P) : On adding AgNO ₃ solution to KCl solution precipitation of AgCl will occur due to which Cl ⁻ already present will be replaced by NO ₃⁻ ions. So conductance of solution will decrease till equivalence point. After complete precipitation of AgCl , further added AgNO ₃ will increase the number of ions in resulting solution so conductance will increase. Option ( Q ) : On adding KCl solution to AgNO ₃ solution precipitation of AgCl will occur due to which already present Ag ⁺ ions will be replaced by K ⁺ ion

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